A) 1.10 V
B) 1.04 V
C) 1.16 V
D) 1.07 V
E) 1.00 V
Correct Answer: D
Solution :
\[C{{u}^{2+}}+2{{e}^{-}}\xrightarrow{{}}Cu\,;\] \[E{}^\circ =0.34\] \[Z{{n}^{2+}}+2{{e}^{-}}\xrightarrow{{}}Zn;\] \[E{}^\circ =-\,0.76\] In the cell, \[Zn\underset{anode}{\mathop{|Z{{n}^{2+}}||}}\,\underset{cathode}{\mathop{Cu|C{{u}^{2+}}}}\,\] In the cell, \[E_{cell}^{\text{o}}=E{{{}^\circ }_{cathode}}-E{{{}^\circ }_{anode}}\] \[0.34-(-\,0.76)=1.1\] \[{{E}_{cell}}=E_{cell}^{\text{o}}-\frac{0.0591}{2}\log \frac{[Z{{n}^{2+}}]}{[C{{u}^{2+}}]}\] \[=1.1-0.02955\,\,\log \frac{0.1}{0.01}\] \[=1.1-0.02955\] \[=1.07\,V\]
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